Question

The octane rating of gasoline is a relationship of the burning efficiency of the given gasoline...

  1. The octane rating of gasoline is a relationship of the burning efficiency of the given gasoline mixture to the burning efficiency of octane (C8H18). Like most of hydrocarbons, octane reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction:

                        C8H18 (l) + O2(g) → CO2 (g) + H2O (g)

If 0.240 mol of octane is allowed to react with 0.890 mol of oxygen gas,

  1. how many moles of water are produced in this reaction (theoretical yield of water)?
  2. How much excess reactant (E.R.) is left in moles?

Homework Answers

Answer #1

The combustion of octane occcurs as follows:
2C8H18 (l) + 25O2(g) → 16CO2 (g) + 18H2O (g)
It is evident from the balanced equation that:
2 mols of C8H18 require 25 mol of O2 to react completely.
1 mol of C8H18 requires 12.5 mol of O2 to react completely.
0.240 mol of C8H18 requires O2 = 12.5 x 0.240 = 3
However, only 0.89 mol of O2 is available.
Hence, O2 is the limiting reagent and C8H18 is the excess reagent.
The quantity of product formed depends on the quantity of the limiting reagent.
25 mol of O2 to react to produce H2O = 18 mol
1 mol of O2 to react to produce H2O = 18/25 mol
0.89 mol of O2 to react to produce H2O = (18/25) x 0.89 = 0.6408 mol
0.89 mol of O2 reacts with C8H18 = (2/25) x 0.89 = 0.0712 mol
Number of moles of (excess reagent) left unreacted = 0.240 -0.0712 = 0.1688 mol

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1.A sample of the male sex hormone testosterone, C19H28O2, contains 3.28×1021 atoms of hydrogen. Q) What...
1.A sample of the male sex hormone testosterone, C19H28O2, contains 3.28×1021 atoms of hydrogen. Q) What is the mass of this sample in grams? 2. The octane rating of gasoline is a relationship of the burning efficiency of the given gasoline mixture to the burning efficiency of octane (C8H18). (Figure 1)Like most hydrocarbons, octane reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is C8H18(g)+O2(g)→CO2(g)+H2O(g) Q) After the reaction, how much octane is...
The octane in gasoline burns according to the following equation: 2C8H18 + 25O2 16CO2 + 18H2O...
The octane in gasoline burns according to the following equation: 2C8H18 + 25O2 16CO2 + 18H2O How many moles of O2 are needed to react fully with 4.99 mol of octane? How many moles of CO2 can form from 0.658 mol of octane? How many moles of water are produced by the combustion of 5.85 mol of octane? If this reaction is used to synthesize 5.42 mol of CO2, how many moles of oxygen are needed? How many moles of...
Gasoline is primarily a mixture of hydrocarbons and is sold with an octane rating that is...
Gasoline is primarily a mixture of hydrocarbons and is sold with an octane rating that is based on a comparison with the properties of isootane (C8H18), which has a molar enthalpy of vaporization of 35.8 kJ/mol and a boiling point of 98.2 degrees celcius. Determine the vapor pressure of isooctane on a very hot summer day when the temperature is 38 degrees celcius.
Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and...
Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . What is the theoretical yield of carbon dioxide formed from the reaction of 2.28g of octane and 14.2g of oxygen gas? Be sure your answer has the correct number of significant digits in it.
Liquid octane (Ch3(CH2)6CH3) reacts with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous...
Liquid octane (Ch3(CH2)6CH3) reacts with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of water formed from the reaction of 5.71g of octan 36.4g of oxygen gas? Be sure your answer has the correct number of significant digits in it.
Here is the combustion reaction for octane (C8H18), which is a primary component of gasoline. How...
Here is the combustion reaction for octane (C8H18), which is a primary component of gasoline. How many moles of CO2 are emitted into the atmosphere when 24.1 g of C8H18 is burned?
1. The combustion of gasoline (C8H18) with excess oxygen produces carbon dioxide and water. -Write a...
1. The combustion of gasoline (C8H18) with excess oxygen produces carbon dioxide and water. -Write a balanced chemical reaction for the combustion of gasoline to yield carbon dioxide and water. -Presuming that a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, determine how many kg of CO2 are produced for each tank of gasoline burned. Also, the products for octane + O2 should be carbon dioxide and water. Now, you have to write it in...
Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and...
Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . Suppose 8.00 g of octane is mixed with 39. g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 3 significant digits.
Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and...
Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . Suppose 9.1 g of octane is mixed with 50.6 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.
Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and...
Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . Suppose 24.0 g of octane is mixed with 29. g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.